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Chemistry > Electronegativity Test > Flashcards

Electronegativity Test Flashcards

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1
Q

what properties can categorize substances?

A

conductivity and dissolving

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2
Q

a substance that does dissolve in water

A

soluble

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3
Q

substance that does not dissolve in water

A

insoluble

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4
Q

conductivity

A

a property that describes how well a substance transmits electricity, heat, or sound

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5
Q

what does electrical conductivity require?

A

the movement of charge as ions or electrons

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6
Q

in the body how does electricity move?

A

as ions, not as electrons

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7
Q

how can conductivity be tested?

A

by setting up an electrical circuit. the wires connect to a battery, the substance, and a light bulb, if the light bulb turns on, it is conductive

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8
Q

substance that dissolves and conducts

A

Ionic, metal and nonmetal atoms

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9
Q

substance that dissolves and doesn’t conduct

A

molecular covalent, nonmetal atoms only (carbon, hydrogen, oxygen)

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10
Q

substance that doesn’t dissolve and conducts

A

metallic, metal atoms only

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11
Q

substance that doesn’t dissolve and doesn’t conduct

A

network covalent, nonmetal atoms only

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12
Q

only substances that contain___ atoms will conduct electricity

A

Metal

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13
Q

substances made entirely out of ___ atoms will not dissolve in water

A

Metal

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14
Q

Many ___ compounds dissolve in water

A

Ionic

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15
Q

what is a chemical bond?

A

the bond that hold atoms together, is the attraction of positive charges in the nucleus and negative charges in the electrons of another atom

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16
Q

Ionic bonding

A
  • Dissolve in water
  • conduct when dissolved
  • tend to be brittle solids
  • made of metal and non metals
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17
Q

Molecular Covalent Bonding

A
  • Some dissolve in water
  • do no conduct
  • some are liquids or gases
  • made entirely of non metal atoms
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18
Q

Metallic Bonding

A
  • Don’t dissolve
  • conducts
  • bendable/ malleable solids
  • made entirely of metal atoms
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19
Q

Network Covalent

A
  • Do not dissolve in water
  • Do not conduct electricity
  • Extremely hard solids
  • Made entirely of non metal atoms
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20
Q

Covalent Bonding

A
  • the nucleus of one atom is attracted to the valence electrons of another atom.
  • one atom doesn’t transfer an electron to the other. both atoms share the valence electron.
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21
Q

in molecular covalent, what do the atoms bond into

A

forms into individual clusters called molecules

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22
Q

in network covalent bonding, how are the valence electrons shared

A

valence electrons are shared between atoms, but form a highly regular extended network, creating a very durable structure

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23
Q

in metallic bonding, the electrons are ___

A
  • distributed around the substance in what is called a sea of electrons.
  • the valence electrons are free to move throughout the substance.
  • they are bonded by the attraction between positively charged atoms and negatively charged “sea” of electrons.
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24
Q

what does conduction require?

A

the movement of a charged particle (ion or electron)

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25
Q

why do metal conduct?

A

the valence electrons can freely move throughout the solid

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26
Q

why do ionic compounds that dissolve conduct

A

because the cations and anions move freely in the solution

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27
Q

why do network covalent solids and molecular covalent substances do not conduct

A

the electrons are stuck between the atoms and are not available to move, so the charge cannot move.

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28
Q

polar molecules are ___ to a charged wand, and ___ smell

A

attracted, Do smell

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29
Q

nonpolar molecules are__ to a charged wand, and __ smell

A

no attracted, Don’t smell

30
Q

Partial charge

A

smaller than the charge on an individual electron or proton

31
Q

when a negative charged wand is next to water, why does it pull towards the water?

A

the molecules in the water orient themselves so that positive is in the direction of the wand, attracting the stream to the wand

32
Q

intermolecular force

A

the attraction between individual molecules in a substance

33
Q

why does water bead up?

A

because it is polar, so they attract to each other

34
Q

why does oil spread out

A

it is nonpolar, they are not attracted to each other, and spread out

35
Q

why is water a liquid and methane a gas at room temperature

A

water is polar, methane is nonpolar. the individual water molecules are attracted to each other and stay as a liquid, the methane attractions are weaker, which means they spread out easier.

36
Q

Methanol dissolves in water, oil does not

A

polar methanol attracts to the polar water molecules. the non polar oil does not attract well with the polar water molecules

37
Q

non polar covalent bonds

A

bonds with the same negativity value

38
Q

polar covalent bonds

A

share electrons unequally, more attracted to one atom (partial)

39
Q

Ionic bonds

A

A large difference in electronegativity, more electronegative ion takes the electrons and becomes a negative ion, the other becomes positive

40
Q

what bonds create dipoles?

A

polar bonds

41
Q

what is a dipole?

A

the polarity of an individual bond between atoms

42
Q

what other properties does polarity effect in a molecule?

A

solubility, smell, boiling and melting points

43
Q

electronegativity

A

the tendency of an atom to attract shared electrons

44
Q

why is a polar molecule called a dipole?

A

because it has 2 poles (+ and - ends)

45
Q

atoms that are more electronegative end up having ____

A

a partial negative charge

46
Q

when is a molecule non polar

A

when 2 atoms with identical electronegativities bond together

47
Q

since CO_2 has 2 dipoles, why isn’t it a polar molecule?

A

the 2 dipoles balance each other, there is no partial positive end to the molecule

48
Q

when 2 atoms with different electronegativities bond together, what is the result? why

A

a polar covalent bond/ because there is a partial negative charge

49
Q

when 2 atoms have identical electronegativities, what is the result? why

A

nonpolar covalent/ there is no partial charge

50
Q

if there is a big difference in the electronegativities of 2 atoms, what is the result? why

A

Ionic bond/ the electronegative pull is so great that it is possible for the electrons to be pulled entirely towards one of the atoms in a bond

51
Q

who proposed the scale for electronegativity

A

Linus Pauling, in 1932

52
Q

what does the electronegativity scale allow you to do?

A
  • compare individual atoms electronegativity/

- the polarity of bonds

53
Q

diatomic molecules

A

molecules with 2 atoms

54
Q

how do you compare the polarity of one bond to another?

A

by looking at the numerical difference between the electronegativities of the 2 atoms

55
Q

bond with a bigger difference in electronegativity between the 2 atoms are_____

A

more polar

56
Q

when the difference between electronegativity between 2 atoms is very large, the bond is considered ___

A

it is no longer considered covalent

57
Q

when 2 atoms are no longer considered covalent, the electrons are transferred from ___ to ____.

A

the less electronegative atom to the more electronegative atom.

58
Q

after the electrons are transfered from one atom to another what forms and what is then created?

A

A cation and anion form and are attracted to one another and then create an ionic bond

59
Q

chemical bond

A

an attraction between atoms that holds them together

60
Q

covalent bonding

A

type of chemical bonding in which 1 or more pairs of valence electrons are shared between the atoms

61
Q

structoral formula

A

OH CH_2 CH_2 CH_2 OH

62
Q

molecular formula

A

C_3 H_8 O_2

63
Q

HONC

A

1234 rule, draw carbon first, then nitrogen, then oxygen, then hydrogen

64
Q

bonded pair

A

pair of electrons that are shared in a covalent bond between 2 atoms

65
Q

lone pair

A

pair of unshared valence electrons that are not involved in bonding in a molecule

66
Q

octet rule

A

non metals combine by sharing electrons so that each atom has a total of eight valence electrons. after bonding, each atom resembles a noble gas in its electron arrangement (8 electrons)

67
Q

diatomic molecule

A

a molecule consisting of 2 atoms

68
Q

how to name an ionic compound

A

METAL AND NON METAL

  • always name cation first (metal) then anion (nonmetal)
  • the cation always stay the same
  • the anion takes the root of the word and then adds “-ide” to the end
    ex: Calcium SulfIDE (CaS)
69
Q

how to name a polyatomic ion

A

SAME AS IONIC EXCEPT:
-the anion name is found on the common ion sheet
-if there are multiple anions, use parenthesis in the formula, to show the polyatomic anion as a single unit, followed by a subscript number
ex: NaNO_3= Sodium Nitrate
MgSO_4 Magnesium Sulfate
(NO “-IDE” IS NEEDED)

70
Q

How to name transition metal cations

A
  • the name of the compound includes a roman numeral to indicate which ion is in the compound
  • the charge of the cation can be determined from the formula by balancing the charge of the anion to give a net charge of zero
    ex: FeO iron(ii) oxide
71
Q

Naming covalent compounds

A

ONLY NONMETALS
-the first element in the formula is named first, and the full element name is used
-the second element is named as though it was an anion
-a prefix is used before the second element, to denote the number of atoms present
-never use mono for the first element
ex: CO_2 carbon monoxide
N_2O_5 dinitrogen pentaoxide
P_4O_6 tetraphosphorus hexoxide

72
Q

Naming Acids

A 
ALWAYS HAVE H IN THEM (except for acetic acid)
- use polyatomic ions to name acids
ex: HCLO_4 Percloric acid
HNO_3 Hydronitric acid 
HCL Hydrocloric acid 
HBr Hydrobromic acid 
H_3PO_4 hydrogen phosphuric acid 
HCLO_2 Hydro Clourous acid 
HCLO_3 chloric acid

Chemistry (10 decks)

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